Chem help Card #2 Mole Problems (Ch 10) Name:______Per______

Topic / Purpose / How / Notes
10.1 – 10.2
Conversions / To change from one label to another / g --can change to – moles g--can change to -- molecules
molecules--can change to – moles g--can change to -- formula units (u)
ect.
1 mole of any gas = 22.4L
Example : Amt given g x (1 mole)_ x (6.02 x 1023 particles)=
1 ---g from periodic table mass 1 mole / DO NOT cross multiply and divide
1) multiply across the top
2) multiply across the bottom
3) divide the top by the bottom.
10.3
% Composition / amount of element in a compound / Use a ratio: Part = %
Whole 100
10.3
Empirical Formula-Molecular Formula / A)
Empirical Formula = “lowest” multiple of any formula—there can be only one
B)
Molecular Formula = Any multiply of an Empirical Formula / Example:
CH5O= Empirical Formula C5H10O5=Molecular Formula
------
40% C = 40g C x 1 mol = 3.33 mol C
12.011 g C
6.67% H = 6.67g H x 1 mol = 6.60 mol H
1.0079 g H
53.3% O = 53.3 g O x 1 mol = 3.33 mol O
15.999 g O
------
Mole Ratio 1 mole C : 2 mole H : 1 mole O
(You can also divide by the smallest mole above to find the ratio)
------
Empirical Formula = CH2O
------
Empirical Formula Mass = 30.0 g/mole (12.011 + 1.0079 + 1.0079 + 15.999)
------
Molar Mass (given in problem) = 150 g/mole = 5
Empirical Formula Mass 30.0 g/mole
------
Molecular Formula = 5 times Empirical Formula = 5 x (CH2O) = C5H10O5 / Steps:
ß
------
1) Change all to moles
------
2) Find the ratio
(divide by the smallest)
------
3) Write the Empirical Formula
------
4) Find the mass of the Empirical Formula
------
5) Get a multiplication factor
------
6) Multiply the Empirical formula
by the factor to get Molecular Formula
Ion (-)


Metal (+) / acetate / bromide / carbonate / chloride / chromate / hydroxide / iodide / nitrate / phosphate / sulfate / sulfide
aluminum / ss / s / n / s / n / i / s / s / i / s / d
ammonium / s / s / s / s / s / s / s / s / s / s / s
barium / s / s / i / s / i / s / s / s / i / i / d
calcium / s / s / i / s / s / ss / s / s / i / ss / d
copper (II) / s / s / i / s / i / i / n / s / i / s / i
iron (II) / s / s / i / s / n / i / s / s / i / s / i
iron (III) / s / s / n / s / i / i / n / s / i / ss / d
lead / s / ss / i / ss / i / i / ss / s / i / i / i
magnesium / s / s / i / s / s / i / s / s / i / s / d
mercury (I) / ss / i / i / i / ss / n / i / s / i / ss / i
mercury (II) / s / ss / i / s / ss / i / i / s / i / d / i
potassium / s / s / s / s / s / s / s / s / s / s / s
silver / ss / i / i / i / ss / n / i / s / i / ss / i
sodium / s / s / s / s / s / s / s / s / s / s / s
zinc / s / s / i / s / s / i / s / s / i / s / i
Abbreviation / Solubility of Matter / State
i / nearly insoluble / (s)
ss / slightly soluble / (s)
s / soluble / (aq)
d / decomposes / (aq)
n / not isolated / (aq)
Evidence of Change

Total Electron Groups / Bonding Groups / Lone Pairs / Electron Geometry / Bond Angle
(degrees) / Molecular Geometry
2 / 1 / 1 / Linear / 180 / Linear
2 / 2 / 0 / Linear / 180 / Linear
3 / 3 / 0 / Trigonal planer / 120 / Trigonal planer
3 / 2 / 1 / Trigonal planer / 120 / Bent
3 / 1 / 2 / Trigonal planer / 180 / Linear
4 / 4 / 0 / Tetrahedral / 109.5 / Tetrahedral
4 / 3 / 1 / Tetrahedral / 107 / Pyramidal
4 / 2 / 2 / Tetrahedral / 105 / Bent

Chem help Card Name:______Per______

Acids / Salts
Hydro___ ic acid / H / a / X / M___ / ide / M / b / X
Hypo___ ous acid / H / a / X / O / n-2 / M Hypo___ / ite / M / b / X / O n-2
___ ous acid / H / a / X / O / n-1 / M___ / ite / M / b / X / O n-1
*___ ic acid / H / a / X / O / n / * M___ / ate / M / b / X / O n
Per_____ ic acid / H / a / X / O / n+1 / M Per___ / ate / M / b / X / O n+1
Common Anions
-1 / -1 / -2
H-1 hydride / HCO3-1 hydrogen carbonate or bicarbonate / O-2 oxide
OH-1 hydroxide / O2-2 peroxide
Cl-1 chloride / S-2 sulfide
CH3COO-1 acetate(C2H3O2) / MnO4-1 permanganate / CrO4-2 chromate
Cr2O7-2 dicromate
(CN)-1 Cyanide / MnO4 -2 Manganate
(SCN)-1 Thiocynate / SiO4-2 Silicate
S2O32- thiosulfate
C2O4 -2 Oxalate
“Ic-Ous” Chart
Stock Name
Metal / Symbols / Traditional
Name
Copper ((I)
Copper II) / Cu1+
Cu2+ / cuprous
cupric
Iron (II)
Iron (III) / Fe2+
Fe3+ / ferrous
ferric
Mercury (I)
Mercury (II) / Hg22+
Hg2+ / mercurous
mercuric
Lead (II)
Lead (IV) / Pb2+
Pb4+ / plumbous
plumbic
Tin (II)
Tin (IV) / Sn2+
Sn4+ / stannous
stannic

REMEMBER:

Chem Is “TRY”

[He] [Ne] [Ar] [Kr] [Xe] [Rn]

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f14 6d10 7p6

2 4 10 12 18 20 30 36 38 48 54 56 70 80 86 88 102 112 118

+1 (-5) (-4) -3 -2 -1

1
H
2.1 / +2 / +3 / +4 / (+5) / 2
He
3
Li
1.0 / 4
Be
1.5 / 5
B
2.0 / 6
C
2.5 / 7
N
3.0 / 8
O
3.5 / 9
F
4.0 / 10
Ne
11
Na
1.0 / 12
Mg
1.2 / 13
Al
1.5 / 14
Si
1.8 / 15
P
2.1 / 16
S
2.5 / 17
Cl
3.0 / 18
Ar
19
K
0.9 / 20
Ca
1.0 / 21
Sc
1.3 / 22
Ti
1.4 / 23
V
1.5 / 24
Cr
1.6 / 25
Mn
1.6 / 26
Fe
1.7 / 27
Co
1.7 / 28
Ni
1.8 / 29
Cu
1.8 / 30
Zn
1.6 / 31
Ga
1.7 / 32
Ge
1.9 / 33
As
2.1 / 34
Se
2.4 / 35
Br
2.8 / 36
Kr
37
Rb
0.9 / 38
Sr
1.0 / 39
Y
1.2 / 40
Zr
1.3 / 41
Nb
1.5 / 42
Mo
1.6 / 43
Tc
1.7 / 44
Ru
1.8 / 45
Rh
1.8 / 46
Pd
1.8 / 47
Ag
1.6 / 48
Cd
1.6 / 49
In
1.6 / 50
Sn
1.8 / 51
Sb
1.9 / 52
Te
2.1 / 53
I
2.5 / 54
Xe
55
Cs
0.8 / 56
Ba
1.0 / 57
La
1.1 / 72
Hf
1.3 / 73
Ta
1.4 / 74
W
1.5 / 75
Re
1.7 / 76
Os
1.9 / 77
Ir
1.9 / 78
Pt
1.8 / 79
Au
1.9 / 80
Hg
1.7 / 81
Tl
1.6 / 82
Pb
1.7 / 83
Bi
1.8 / 84
Po
1.9 / 85
At
2.1 / 86
Rn
87
Fr
0.8 / 88
Ra
1.0 / 89
Ac
1.1
H2
N2 / O2 / F2
If these gases are by themselves they are diatomic / Cl2
Br2
I2

p+

Prefixes for naming Method 2
Mono / 1 / Hepta / 7
Di / 2 / Oxo / 8
Tri / 3 / Nona / 9
Tetra / 4 / Deca / 10
Penta / 5 / Undeca / 11
Hexa / 6 / Dodeca / 12

SUBSTANCE #1 Avo #

GAW 6.02 x 1023

gms moles particles

coefficients of coefficients of BCE BCE

SUBSTANCE #2

GAW

gms moles particles

Avo # 6.02 x 1023